Standard electrode potential data are useful for understanding the suitability of an…

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration.  Some half cell reactions and their standard potentials are given as follows:

\[\begin{array}{l} \mathrm{MnO}_{4}^{-}(\mathrm{aq})+8 \mathrm{H}^{+}(\mathrm{aq})+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \mathrm{E}^{\mathrm{a}}=1.51 \mathrm{~V} \\ \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+14 \mathrm{H}^{+}(\mathrm{aq})+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \mathrm{E}^{\mathrm{a}}=1.38 \\ \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+}(\mathrm{aq}) \mathrm{E}^{\mathrm{a}}=0.77 \mathrm{~V} \\ \mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-}(\mathrm{aq}) \mathrm{E}^{\mathrm{a}}=1.40 \mathrm{~V} \end{array}\]